S2

Question 1

What is a metallic bond?

Answer 1

A metallic bond is the electrostatic attraction between a lattice of positive metal ions and delocalized electrons.

Question 2

Why do metals conduct electricity?

Answer 2

Because of the presence of delocalized electrons that can move freely throughout the metal structure.

Question 3

Why do metals conduct heat well?

Answer 3

Delocalized electrons transfer thermal energy rapidly through the structure.

Question 4

Why are metals malleable?

Answer 4

The layers of metal ions can slide over each other while remaining bonded by delocalized electrons.

Question 5

How does ion charge affect metallic bond strength?

Answer 5

Higher charge increases electrostatic attraction, strengthening the bond.

Question 6

How does ion size affect metallic bond strength?

Answer 6

Smaller ions pack more closely, increasing bond strength.

Question 7

What trend is seen in melting points of s and p block metals?

Answer 7

Generally, melting points increase with increasing charge and decrease with increasing atomic radius.

Question 8

What is special about d-electrons in transition metals?

Answer 8

They are delocalized and contribute to bonding, conductivity, and magnetism.

Question 9

Why do transition metals have high melting points?

Answer 9

Due to strong metallic bonding involving d-electrons.

Question 10

Why do transition metals conduct electricity?

Answer 10

Delocalized d-electrons move freely to conduct electricity.

Question 11

What is a covalent bond?

Answer 11

A covalent bond is the sharing of electron pairs between atoms.

Question 12

What is the octet rule?

Answer 12

Atoms tend to form bonds to achieve 8 electrons in their valence shell.

Question 13

How do you deduce Lewis structures for simple molecules?

Answer 13

By arranging electrons to satisfy the octet rule using single, double, or triple bonds.

Question 14

What is a single bond?

Answer 14

A bond formed by one shared pair of electrons.

Question 15

What is a double bond?

Answer 15

A bond formed by two shared pairs of electrons.

Question 16

What is a triple bond?

Answer 16

A bond formed by three shared pairs of electrons.

Question 17

How does bond number affect bond length and strength?

Answer 17

More bonds = shorter and stronger bond.

Question 18

What is a coordination bond?

Answer 18

A bond where both electrons come from the same atom (common in metal complexes).

Question 19

What does VSEPR stand for?

Answer 19

Valence Shell Electron Pair Repulsion.

Question 20

How does VSEPR predict shape?

Answer 20

By minimizing repulsion between electron domains.

Question 21

How do lone pairs affect bond angles?

Answer 21

Lone pairs repel more strongly and reduce bond angles.

Question 22

How do you determine bond polarity?

Answer 22

By comparing the electronegativity of the bonded atoms.

Question 23

What is a dipole moment?

Answer 23

A measure of the polarity of a molecule based on the vector sum of bond dipoles.

Question 24

What are key carbon allotropes?

Answer 24

Diamond, graphite, fullerenes, graphene.

Question 25

What are properties of silicon dioxide?

Answer 25

High melting point, hard, does not conduct electricity.

Question 26

What are London dispersion forces?

Answer 26

Weak attractions due to temporary dipoles.

Question 27

What are dipole–dipole forces?

Answer 27

Attractions between polar molecules.

Question 28

What is hydrogen bonding?

Answer 28

Strong dipole interaction involving H bonded to N, O, or F.

Question 29

How do you determine the type of IMF?

Answer 29

Based on molecular polarity and presence of H-bonding atoms.

Question 30

How do IMF affect physical properties?

Answer 30

Stronger IMFs result in higher boiling/melting points.

Question 31

What is chromatography?

Answer 31

A technique to separate substances based on solubility and intermolecular forces.

Question 32

What is Rf value?

Answer 32

Distance moved by substance / distance moved by solvent.

Question 33

What are resonance structures?

Answer 33

Multiple Lewis structures representing delocalized electrons.

Question 34

How is benzene structured?

Answer 34

Six carbon ring with delocalized π electrons, equal bond lengths.

Question 35

What are expanded octets?

Answer 35

Species where central atom has more than 8 electrons, common in period 3+.

Question 36

What is a sigma bond?

Answer 36

A bond formed by head-on overlap of orbitals.

Question 37

What is a pi bond?

Answer 37

A bond formed by sideways overlap of p orbitals.

Question 38

What is hybridization?

Answer 38

Mixing of atomic orbitals to form new hybrid orbitals.

Question 39

What geometry is predicted by sp3 hybridization?

Answer 39

Tetrahedral.

Question 40

What geometry is predicted by sp2 hybridization?

Answer 40

Trigonal planar.

Question 41

What geometry is predicted by sp hybridization?

Answer 41

Linear.

Question 42

How to predict ion charge from electron configuration?

Answer 42

Atoms lose/gain electrons to achieve noble gas configuration.

Question 43

How do ionic bonds form?

Answer 43

From the electrostatic attraction between cations and anions.

Question 44

How to name ionic compounds?

Answer 44

Combine the names of cation and anion.

Question 45

What is the formula of ammonium?

Answer 45

NH4+

Question 46

What is the formula of hydroxide?

Answer 46

OH–

Question 47

What is the formula of nitrate?

Answer 47

NO3–

Question 48

What is the formula of hydrogencarbonate?

Answer 48

HCO3–

Question 49

What is the formula of carbonate?

Answer 49

CO32–

Question 50

What is the formula of sulfate?

Answer 50

SO42–

Question 51

What is the formula of phosphate?

Answer 51

PO43–

Question 52

Why do ionic compounds have high melting points?

Answer 52

Strong electrostatic forces require lots of energy to break.

Question 53

Why do ionic compounds conduct electricity in solution?

Answer 53

Ions are free to move and carry current.

Question 54

Why are ionic compounds soluble in water?

Answer 54

Water molecules surround and separate the ions.

Question 55

What is lattice enthalpy?

Answer 55

The energy released when one mole of an ionic solid is formed from its ions.

Question 56

What is the bonding continuum?

Answer 56

Range from ionic to covalent to metallic bonding.

Question 57

How does electronegativity affect bonding?

Answer 57

Greater difference → more ionic character.

Question 58

What does the bonding triangle show?

Answer 58

Position of a compound between ionic, covalent, and metallic bonding.

Question 59

What is an alloy?

Answer 59

A mixture of a metal with other elements.

Question 60

What are properties of alloys?

Answer 60

Stronger, corrosion-resistant, variable properties.

Question 61

Give examples of alloys.

Answer 61

Bronze, brass, stainless steel.

Question 62

What is a polymer?

Answer 62

A large molecule made of repeating monomers.

Question 63

How does polymer structure affect properties?

Answer 63

Cross-linking and branching affect flexibility and melting point.

Question 64

What are addition polymers?

Answer 64

Polymers formed by addition reactions of alkenes.